1 / 10

Bond Order, Length, and Energy

Bond Order, Length, and Energy. Bond Order. The number of bonding electron pairs shared by two atoms in a molecule. Can be whole numbers as well as fractional numbers. Draw H2, NH3, and CH4. Each have a bond order of 1 Draw CO2 and C2H4

jbarlow
Télécharger la présentation

Bond Order, Length, and Energy

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Bond Order, Length, and Energy

  2. Bond Order • The number of bonding electron pairs shared by two atoms in a molecule. • Can be whole numbers as well as fractional numbers. • Draw H2, NH3, and CH4. • Each have a bond order of 1 • Draw CO2 and C2H4 • The C=O bond in CO2 has a bond order of 2, as does the C=C bond in C2H4. • Draw N2 and CO • Bond orders of 3

  3. Bond Order • Draw O3 • It has 2 resonance structures, so how do I calculate the bond order? • Bond Order = _[Number of shared pairs in all X-Y bonds]_ [Number of X-Y links in the molecule or ion] • Bond Order = _[Number of bonds]_ [Number of structures] • Each O-O bond has a total of 3 shared pairs/2 structures • Bond Order = 1.5

  4. Bond Order • Draw C2O4-2 … • How many resonance structures are there? • What’s the bond order between Carbon and Oxygen? • Draw OCN- … • How many resonance structures are there? • What’s the bond order between C and O? C and N?

  5. Bond Length • Is the distance between the nuclei of two bonded atoms. • Related to 2 things: • Size of the atom • The larger the atom, the longer the bond • H-F < H-Cl < H-Br < H-I • Bond Order • When comparing bonds between the same two atoms, the larger the bond order, the shorter the bond • C-O > C= O > C= O • Single bonds are longer than double bonds, which are longer than triple bonds

  6. Bond Length • Compare the bond lengths between carbon monoxide, carbon dioxide, and carbonate ion. Arrange them in order of increasing bond length. • Carbon Monoxide < Carbon Dioxide < Carbonate Ion Bond order: 3 2 1.3

  7. Bond Enthalpy • Bond Dissociation Enthalpy • the enthalpy change for breaking a bond in a molecule with the reactant and products in the gas phase • Enthalpy (ΔH) • The process of breaking bonds in a molecule is always endothermic • ΔH is positive. Energy must be put in to break a bond. • The process of forming bonds in a molecules is always exothermic • ΔH is negative. Energy is released when a bond is formed

  8. Bond Enthalpy ΔHrxn = [∑(Bond enthalpies bonds broken)] – [∑(Bond enthalpies bonds formed)] or ΔHrxn = [∑ ΔHbonds broken ] – [ ∑ ΔHbonds formed]

  9. Practice Problems • Compare the nitrogen-nitrogen bond in hydrazine, H2NNH2, with that in “laughing gas”, N2O. In which molecule is the nitrogen-nitrogen bond shorter? In which is the bond stronger?

  10. Practice Problems • The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water. OF2(g) + H2O(g)  O2(g) + 2HF(g) ΔHrxn = -318kJ/mol●rxn Using bond dissociation enthalpies, calculate the bond dissociation energy of the O-F bond OF2. H-O = 463 kJ/mol O=O = 498 kJ/mol H-F = 565 kJ/mol

More Related